Given that the solubility product constant (Ksp) of C2D3 is 9.14 × 10^{-9}, what is the molar solubility of C2D3 in mol/L?

• A. 1.32 × 10^{-2} mol/L
• B. 1.32 × 10^{-3} mol/L
• C. 1.32 × 10^{-3} mol/L
• D. 1.32 × 10^{-2} mol/L

Answer: (B)

Verified step by step guidance

1. Identify the dissociation equation of the compound C2D3 in water. For example, if C2D3 dissociates as C2D3 (s) \rightarrow C^{+} + D_3^{-}, then the molar solubility is represented by the concentration of ions produced.
2. Express the solubility product constant (K_{sp}) in terms of the molar solubility (s). For a salt that dissociates into one cation and one anion, K_{sp} = [C^{+}][D_3^{-}] = s \times s = s^{2}.
3. Set up the equation using the given K_{sp} value: s^{2} = 9.14 \times 10^{-9}.
4. Solve for the molar solubility s by taking the square root of both sides: s = \sqrt{9.14 \times 10^{-9}}.
5. Interpret the result as the molar solubility of C2D3 in mol/L, which represents the maximum concentration of C2D3 that can dissolve in water at equilibrium.